Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 13: Q98P (page 562)

What is the freezing point of 0.251 m urea in water?

Short Answer

Expert verified

The freezing point is-0.664°C

Step by step solution

01

Concept

The freezing point of a solution containing a non-volatile solute is lower than the freezing point of a pure solvent. The depression in the freezing point can be calculated as:

ΔTf=iKfm

where the Kfis the molal freezing point depression constant and its value is equal to1.86C°/mfor aqueous solutions. The mis the molality of the particles, the iis the van’t Hoff factor, and its value for 1 urea is 1 because a urea is a non-electrolyte substance and it does not dissociate into ions in a solution

02

Calculate the depression in freezing point for urea (ΔTf)

∆Tf=iKfm=1.86°C/m×0.251m=0.466°C

03

Freezing point of solution

ΔTf=Tsolvent-TsolutionTsolvent=0°C0°C-Tsolution=0.466°CTsolution=-0.466°C.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Four Utubes each have distilled water in the right arm, a solution in the left arm, and a semipermeable membrane between arms.

  1. If the solute is KCl, which solution is most concentrated?
  2. If each solute is different but all the solutions have the same molarity, which contains the smallest number of dissolved ions?

How many moles of solute particles are present in 1 mL of each of the following aqueous solutions?

(a)0.02M CuSO4

(b)0.004 MBa(OH)2

(c)0.08 M pyridine (C5H5N)

(d) 0.05 M (NH4)2CO3

Calculate the molarity of each aqueous solution:

  1. 0.82 g of ethanol (C2H5OH) in 10.5 mL of solution
  2. 1.27 g of gaseous NH3 in 33.5 mL of solution.

Name three intermolecular forces that stabilize the shape of a soluble, globular protein, and explain how they act.

Which solution has the higher boiling point?

(a) 38.0 g of C3H8O3 in 250. g of ethanol or 38.0 g of C2H6O2in 250. g of ethanol

(b) 15 g of C2H6O2 in 0.50 kg of H2O or 15 g of NaCl in 0.50 kg of H2O.
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Analysis

Read Explanation

Chemistry Branches

Read Explanation

Organic Chemistry

Read Explanation

Kinetics

Read Explanation

Making Measurements

Read Explanation

Ionic and Molecular Compounds

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free